Answer
$2H_{2}O(l)\rightarrow 2H_{2}(g)+O_{2}(g)$
Reactant-favored
Work Step by Step
The equation for water getting decomposed to hydrogen and oxygen can be written as
$H_{2}O(l)\rightarrow H_{2}(g)+O_{2}(g)$
The balanced form of the above equation is
$2H_{2}O(l)\rightarrow 2H_{2}(g)+O_{2}(g)$. As this reaction has virtually no tendency to occur by itself, the process is reactant-favored. That is reactant water predominate over products.
